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13 August, 17:41

Part 1. Determine the molar mass of a 0.458-gram sample of gas having a volume of 1.20 L at 287 K and 0.980 atm. Show your work. Part 2. If this sample was placed under extreme pressure, describe how the actual volume would compare to the predicted volume. Explain your answer.

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  1. 13 August, 17:45
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    Part 1: 9.165 g/mol.

    Part 2: The volume will decrease.

    Explanation:

    Part 1:

    To solve this problem, we can use the general gas law:

    PV = nRT,

    where, P is the pressure of the gas (atm) (P = 0.98 atm).

    V is the volume of the gas (L) (V = 1.2 L).

    n is the no. of moles of the gas (mol).

    R is the general gas constant (R = 0.082 L. atm/mol. K).

    T is the temperature of the gas (K) (T = 287 K).

    ∴ n = PV/RT = (0.98 atm) (1.2 L) / (0.082 L. atm/mol. K) (287 K) = 0.0499 mol ≅ 0.05 mol.

    ∵ n = mass/molar mass

    ∴ molar mass = mass/n = (0.458 g) / (0.05 mol) = 9.165 g/mol.

    Part 2:

    The volume of the gas will decrease as the sample is placed under extreme pressure.

    Boyle's Law states that at constant temperature, the volume of a given quantity of a gas varies inversely with its pressure.

    P ∝ 1/V.

    so, as the sample is placed under extreme pressure, the volume of the gas will be decreased.
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